Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g).

2SO2(g)+O2(g)=2SO3(g) Kc=1.7*10^8
[SO3]aq=0.0034 M
[O2]aq=0.0018 M

To determine the equilibrium concentration of SO2(g), we can use the equation and the equilibrium constant (Kc) for the reaction.

The balanced chemical equation for the reaction is:

2 SO2(g) + O2(g) ⇌ 2 SO3(g)

The equilibrium constant expression based on the stoichiometry is:

Kc = [SO3(g)]^2 / ([SO2(g)]^2 * [O2(g)])

Given that [SO3(g)] = 0.0034 M and [O2(g)] = 0.0018 M, we can substitute these values into the equation:

1.7 * 10^8 = (0.0034)^2 / ([SO2(g)]^2 * 0.0018)

To solve for [SO2(g)], we rearrange the equation and isolate [SO2(g)]:

[SO2(g)]^2 = [(0.0034)^2 * 0.0018] / 1.7 * 10^8

Taking the square root of both sides, we get:

[SO2(g)] = √([(0.0034)^2 * 0.0018] / 1.7 * 10^8)

Calculating this value will give you the equilibrium concentration of SO2(g) at the given temperature.

To determine the equilibrium concentration of SO2(g), we can use the equilibrium constant expression and the given equilibrium concentrations of SO3(g) and O2(g).

The equilibrium constant expression for the given reaction is:
Kc = [SO3(g)]^2 / ([SO2(g)]^2 * [O2(g)])

We are given:
[SO3(g)] = 0.0034 M
[O2(g)] = 0.0018 M
Kc = 1.7 * 10^8

Let's plug in the values into the equilibrium constant expression and solve for [SO2(g)].

Kc = (0.0034 M)^2 / ([SO2(g)])^2 * (0.0018 M)
1.7 * 10^8 = 0.0034^2 / ([SO2(g)])^2 * 0.0018

Now, let's rearrange the equation to solve for [SO2(g)].

([SO2(g)])^2 = (0.0034^2 * 0.0018) / (1.7 * 10^8)
([SO2(g)])^2 = 0.00000220492 / (1.7 * 10^8)
([SO2(g)])^2 = 1.2964 * 10^-14

Now, take the square root of both sides to find [SO2(g)].

[SO2(g)] = sqrt(1.2964 * 10^-14)
[SO2(g)] = 1.14 * 10^-7 M

Therefore, the equilibrium concentration of SO2(g) is 1.14 * 10^-7 M.

K=[SO3]^2 /[O2][SO2]^2

Put in the numbers, solve for the concentration of SO2

1.9M